The standard entroples of `N_(2)(g), H_(2) (g) and NH_(3) (g)` are `191.5, 130.5, 192.6 Jk^(-1) mol ^(-1)`. The value of `DeltaS^(@)` of formation of ammonia is

The standard entropies of N_(2)(g),H_(2)(g) and NH_(3)(g) are 191.5, 192.6JK^(-1)mol^(-1) . The value of DeltaS^(0) during the formation of 1 mole of ammonia is

The standard enthyalpy of N_(2(g))+3H_(2(g)rarr2NH_(3(g)) is

Calculate the value of log K_(p) for the reaction, N_(2(g))+3H_(2(g))hArr2NH_(3(g)) at 25^(@)C . The standard enthalpy of formation of NH_(3(g)) is -46kJ and standard entropies of N_(2(g)) , H_(2(g)) and NH_(3(g)) are 191 , 130 , 192 JK^(-1) mol^(-1) . respectively. ( R=8.3JK^(-1)mol^(-1) )

Consider the synthesis of ammonia: {:(N_(2) (g) + 3 H_(2) (g) rarr 2NH_(3) (g),,,Delta_(r )H^(@)=-92.6 kJ):} If absolute entropies of N_(2) (g), H_(2) (g) , and NH_(3) (g) are 192 j K^(-1) mol^(-1), 131 jK^(-1) mol^(-1) , and 193 j k^(-1) , respectively, at 25^(@)C , predict whether the reaction is spontaneous or not. Strategy : Calculate Delta S_("univ") using Delta S_("says") and Delta S_("surr") . For calculating Delta S_("rays") use the absolute entropies of reactants and product. For calculating Delta S_("surr") , use Delta_(r) H^(@) and T .

Given: N_(2)(g) + 3H_(2)(g) to 2NH_(3)(g), Delta_(r)H^(@) = -924 kJ "mol"^(-1) . What is the standard enthalpy of formation of NH_(3) gas?